水的化学
Contents
水的化学
水的化学
以通过考试为目的,因为我的未来和我的化学无关。
我不喜欢无意义的中英文混杂。但是因为我的未来与化学无关,所以去他丫的。
第六章 原子结构
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Electronic radiation(电磁辐射)
- 由一些电磁过程而放出的电磁辐射。
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The speed of light(光速)
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Periodic(周期性)
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$\lambda \cdot \nu = c$
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电磁波谱
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Quantum(量子)
- 最小的能量单位
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Photoelectric effect(光电效应)
- A minimum frequency of light, different for different metals, is required for the emission of electrons.
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Work function
- A certain amount of energy that required for the electrons to overcome the attractive forces holding them in the metal.
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Wave-particle duality(波粒二象性)
- Spectrum(光谱)
- Monochromatic (单色的)
- Polychromatic (复色的)
- Continuous spectrum(连续谱)
- Line spectrum (线状谱)
- Spectrum(光谱)
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波尔模型
- $\displaystyle E = -hcR_H\frac{1}{n^2}=-2.18\times {10}^{-18}\frac{1}{n^2}$ 仅仅适用于氢原子
- Ground state:基态
- Excited state:激发态 n=2或者更高
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Matter Waves物质波
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Uncertainty principle不确定性原理
- $\begin{aligned} \Delta x \cdot \Delta(mv) \geq \frac{h}{4\pi} \end{aligned}$
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Wave Function(波函数)
- a series of mathematical functions that describe the electron in the atom.
- 一系列描述原子中的电子的函数
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Probabiliy density
- $\Phi ^2$, 一个电子在给定位置出现的概率
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Orbital
- 一组波函数,由薛定谔方程的解产生。每个轨道都有一个特有的形状和能量。
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The principal quantum number($n$)(主量子数)
- energy level(能级),n=1,2,3,4
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The angular momentum quantum number($l$)
- Shape of orbital, $l=0,1,…,n-1$
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The magnetic quantum number($m_l$)
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Orientation(控制轨道的指向),$m_{l} = \text{interval of } [-l,l]$
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Values of $n$ 1$\quad$ 2$\quad$ 3$\quad$ 4$\quad$ Letter used K L M N Values of $l$ 0$\quad$ 1$\quad$ 2$\quad$ 3$\quad$ Letter used s p d f
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Electron Shell(电子层)
- the collection of orbitals with the same value of n
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Subshell(亚层)
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degenerate(简并)
- 能量相同
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electron spin
- 电子自旋,仿佛在转
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The spin magnetic quantum number($m_{s}$)
- 和其他三个量子数无关,它永远取正或者负二分之一
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Electron configuration(电子构型)
- 电子填充轨道的方式
- The most stable electron configuration-the ground state-is that in which the electrons are in the lowest possible energy status
- The orbitals are filled in order of increasing energy, with no more than two electrons per orbital
- 电子填充轨道的方式
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Orbital diagram
- Each orbital is denoted by a box and each electron by a half arrow
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The Pauli exclusion principle
- an orbital can hold a maximum of two electrons and they must have opposite spins.
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Hund’s rule:
- For degenerate orbitals, the lowest energy state is attained when the number of electrons having the same spin is maximized.
- The rule: filling up of the orbitals is dependent on orbital energy while removal of electrons from orbitals is dependent on orbital location.